Studied by 1 person
Acids Individual Properties
Taste sour
Can sting or burn skin
React with metals
Has a pH<7
Turns blue litmus paper red
Bases Individual Properties
Taste bitter
Feel slippery on skin
Do NOT react with metals
Has a pH>7
Turns red litmus paper blue
Both Acids and Bases
Conduct electricity
Can neutralize each other
An acidic solution contains
more H+ ions than OH- ions
A basic solution contains
more OH- than H+ ions
When dissolved in water
Bases produce OH-
Acids produce H+
Phenolphthalein
Acids are colorless
Bright pink in bases
pH
Power of Hydrogen (H+)
All water solutions
contain OH- and H+ ions
Bronsted-Lowry Theory
States that an acid is always a hydrogen ion donor and a base is always a hydrogen ion accepter.
Conjugate Acid
A substance produced when a base accepts an H+ ion, the reaction can be reversed by the conjugate acid donating its H+
Conjugate Base
A substance produced when an acid donates an H+ ion, the reaction can be reversed by the conjugate base accepting an H+
Titration
Procedure to determine the concentration of a solution with a known volume using a solution of known concentration with a burette
Standard Solution
The solution of known concentration
Equivalence Point
When the concentration of H+ from the acid are equal to the concentration of OH- from the base, the solution remains colorless.
End Point
One drop past the equivalence point, the solution is slightly basic so the solution changes to a pink with the phenolphthalein
Neutralization
Concentration of the acid equals the concentration of the base: H+ = OH-
Each increase in one unit of pH is
a 10x decrease in H+ ions (logarithmic)
pH formula
pH = -log[H+]
pH + pOH formula
pH + pOH = 14.00
pOH formula
pOH = -log[OH-]
pOH scale
Power of Hydroxide 14-0
[H+] formula
[H+]=10^-pH
[OH-] formula
[OH-]=10^-pOH
